Define the equilibrium constant kp for the reaction

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Reference no: EM13221865

Having problems with this particular problem. I'm setting up the equation using a chart my professor showed me but I can't get a reasonable answer, they keep coming out to be negative when it shouldn't be.

Consider the following reversible homogeneous reaction:

C(s) + CO2(g) <=> 2CO(g)
At 700 degrees C, the total pressure of the system is found to be at 3.45 atm. If the equilibrium constant Kp fo rthis reaction is equal to 1.52, calculate the equlibrium partial pressures of CO2 and CO gases.

Reference no: EM13221865

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